determine whether the following salts will form acidic, neutral or basic solutions in water.
Na2HPO4
CaNO2
NH4CH3COO
Al2SO4
NaF
Please, i need the answer to this question within 2 hours of when i post this!
Some of the formulae are incorrect.
You need to decide if the salts are salts of
weak acid + strong base => basic solution
strong acid + weak base => acidic solution
strong acid + strong base => neutral solution
To determine whether the given salts will form acidic, neutral, or basic solutions in water, we need to analyze the ions they dissociate into in water. From there, we can identify the acidic or basic nature of these ions.
1. Na2HPO4:
When Na2HPO4 dissociates in water, it forms Na+ ions and HPO4^2- ions. The HPO4^2- ion can act as a weak base, making the solution slightly basic.
2. Ca(NO2)2:
Calcium nitrite, Ca(NO2)2, dissociates into Ca^2+ ions and NO2^- ions. Neither of these ions are known to be acidic or basic. Therefore, the solution is likely to be neutral.
3. NH4CH3COO:
Ammonium acetate, NH4CH3COO, dissociates into NH4+ ions and CH3COO^- ions. The NH4+ ion can act as a weak acid, making the solution slightly acidic.
4. Al2(SO4)3:
Aluminum sulfate, Al2(SO4)3, dissociates into Al^3+ ions and SO4^2- ions. Neither of these ions are acidic or basic. Therefore, the solution is likely to be neutral.
5. NaF:
Sodium fluoride, NaF, dissociates into Na+ ions and F- ions. The F- ion is the conjugate base of a weak acid (HF) and can act as a weak base, making the solution slightly basic.
In summary:
- Na2HPO4 forms a basic solution.
- Ca(NO2)2 forms a neutral solution.
- NH4CH3COO forms an acidic solution.
- Al2(SO4)3 forms a neutral solution.
- NaF forms a basic solution.
Remember, the classifications provided above (acidic, neutral, basic) are relative, and these solutions will not be strongly acidic or basic unless they are highly concentrated.